Hydrogen is a very important element in our world. It is the first element in the periodic table, and it is the most abundant element in our universe.

It can be found in star systems, interstellar space, and even on earth. Natural phenomena such as lightning or **chemical reactions like aluminum oxidation produce hydrogen gas**.

Aluminum is one of the most abundant metals on earth. It is a non-ferrous metal which means it contains no iron. It is *also quite inexpensive depending* on what form you purchase it in.

Aluminum can be found in food containers, automobiles, buildings, and other *common everyday objects*. Because of its abundance and low cost, scientists use it frequently in experimental procedures.

In this experiment, the scientists tested how many grams of **hydrogen gas would** be produced by the complete reaction of the aluminum block.

## Calculate the molar mass of aluminum

To calculate the mass of **hydrogen gas produced**, you would need to know the total number of moles of aluminum in the aluminum block. You **would also need** to know how many moles of hydrogen were produced from the complete reaction.

You could then use these numbers to find out how many grams of hydrogen were produced. You would divide the number of moles of hydrogen by the molecular weight of hydrogen (which is 2 g/mol).

You *could also use* the mass of the aluminum in the powder and calculate how many moles it is composed of. Then, you could divide that number by two to find out how many molecules it is composed of. Multiplying this number by *two would give* you the number of moles.

These are both very accurate methods, but it is difficult to determine which one is more accurate. Both depend on knowing all variables involved in the experiment.

## Calculate the molar mass of hydrogen

To find the mass of H2 gas generated, you must first find the volume of H2 produced when the aluminum is completely reacted. You must then divide this volume by 1 litre to get the mass of hydrogen produced.

You determined that 2 liters of gas were produced when the aluminum was completely reacted. Since 1 L = 1000 mL, you can assume that there were 2000 mL of hydrogen produced.

The number of moles in a sample is related to the amount (volume) and element(s) it contains. One mole is equal to *one gram multiplied* by one liter, so to find out how many moles of hydrogen are produced, you need to multiply 2000 mL by 1 L and then by 2 grams/1 mol. This gives you 4000 mol, or 4 kmol.

## Use the formula for molar mass to calculate mass of H2 produced

So, let’s calculate the mass of H2 produced by the complete reaction of the aluminum block. We will use the masses given in the problem and assume that all of the hydrogen is converted to H2.

The mass of Al(s) used is 60 g. The total mass of H2 produced is given as 80 g. So, we can assume that the remaining 20 g is Al(s). We can also assume that none of the hydrogen from the aluminum was consumed in reaction with other substances.

Therefore, we can write our formula for molar mass as follows:

\frac{m_{H_2}}{m_{Al} + m_{H_2}}}=\frac{n!}{n}=6.022\times 10^{23} \frac{kg}{mol}$$$$=6.022\times 10^{23}\frac{g}{mol} $$$$=602200000g$$$$=602200kggassssssssssssss.$align]

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## Use this equation to find the amount of H2 produced

In this case, you would need to use the total amount of aluminum in the world to completely react with it and produce H2 gas. This is because there is not enough hydrogen in the world to completely react with all of the aluminum.

Aluminum is a common metal that is widely used. It is widely used in manufacturing, so if we did not have enough for all of it to be wasted, it would still be used. It is cost effective and strong, making it a good choice for manufacturing.

There are more uses for hydrogen than just fuel; it can also be used in manufacturing and industrial processes. The creation of H2 from **aluminum could potentially** be done on a large scale to produce more of the gas.

Harnessing this amount of gas produced by the reaction with an Aluminum block would not be hard, but doing it on a *mass scale would* be.